chapter 17 · pdf filechapter 17 spontaneity ... section 17.1 spontaneous processes and...

Chapter 17

Spontaneity, Entropy,

and Free Energy

Section 17.1 Spontaneous Processes and Entropy

http://www.bozemanscience.com/ap-chemistry/

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2013 AP Curriculum Guidelines

Thermodynamics vs. Kinetics

Domain of Kinetics

Rate of a reaction depends on the pathway from reactants to products.

Thermodynamics tells us whether a reaction is spontaneous based only on the properties of reactants and products.

Spontaneous Processes and Entropy

Thermodynamics lets us predict the direction in which a process will occur but gives no information about the speed of the process.

A spontaneous process is one that occurs without outside intervention.

Thermodynamically favorable

Consider 2.4 moles of a gas contained in a 4.0 L bulb at a constant temperature of 32°C. This bulb is connected by a valve to an evacuated 20.0 L bulb. Assume the temperature is constant.

a) What should happen to the gas when you open the valve?

CONCEPT CHECK!

b) Calculate ΔH, ΔE, q, and w for the process you described above.

All are equal to zero.

CONCEPT CHECK!

c) Given your answer to part b, what is the driving force for the process?

Entropy

CONCEPT CHECK!

The Expansion of An Ideal Gas Into an Evacuated Bulb

Entropy

The driving force for a spontaneous process is an increase in the entropy of the universe.

A measure of molecular randomness or disorder.

Entropy

Thermodynamic function that describes the number of arrangements that are available to a system existing in a given state.

Nature spontaneously proceeds toward the states that have the highest probabilities of existing.

The Microstates That Give a Particular Arrangement (State)

Positional Entropy

A gas expands into a vacuum to give a uniform distribution because the expanded state has the highest positional probability of states available to the system.

Therefore: Ssolid < Sliquid << Sgas

Predict the sign of ΔS for each of the following, and explain:

a) The evaporation of alcohol

b) The freezing of water

c) Compressing an ideal gas at constant temperature

d) Heating an ideal gas at constant pressure

e) Dissolving NaCl in water

CONCEPT CHECK!

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2014 AP Exam

Section 17.2 Entropy and the Second Law of Thermodynamics

Second Law of Thermodynamics

In any spontaneous process there is always an increase in the entropy of the universe.

The entropy of the universe is increasing.

The total energy of the universe is constant, but the entropy is increasing.

Suniverse = ΔSsystem + ΔSsurroundings

ΔSsurr

ΔSsurr = +; entropy of the universe increases

ΔSsurr = -; process is spontaneous in opposite direction

ΔSsurr = 0; process has no tendency to occur

2014 AP Exam

Section 17.3 The Effect of Temperature on Spontaneity

For the process A(l) A(s), which direction involves an increase in energy randomness? Positional randomness? Explain your answer.

As temperature increases/decreases (answer for both), which takes precedence? Why?

At what temperature is there a balance between energy randomness and positional randomness?

CONCEPT CHECK!

Since energy is required to melt a solid, the reaction as written is

exothermic. Thus, energy randomness favors the right (product;

solid). Since a liquid has less order than a solid, positional

randomness favors the left (reactant; liquid).

CONCEPT CHECK!

Describe the following as spontaneous/non-spontaneous/cannot tell, and explain.

A reaction that is:

a) Exothermic and becomes more positionally random

Spontaneous

b) Exothermic and becomes less positionally random

Cannot tell

a) Endothermic and becomes more positionally random

Cannot tell

a) Endothermic and becomes less positionally random

Not spontaneous

Explain how temperature affects your answers.

CONCEPT CHECK!

ΔSsurr

The sign of ΔSsurr depends on the direction of the heat flow.

The magnitude of ΔSsurr depends on the temperature.

ΔSsurr

Heat flow (constant P) = change in enthalpy = ΔH

surr =

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Section 17.4 Free Energy

Free Energy (G)

A process (at constant T and P) is spontaneous in the direction in which the free energy decreases.

Negative ΔG means positive ΔSuniv.

univ = (at constant and )

S T PT

Gibbs Free Energy (G)

ΔG = ΔH – TΔS (at constant T and P)

Energy Free to do work

2014 AP Exam

Hint: Which equation should you use?

2014 AP Exam

Section 17.4 Free Energy A liquid is vaporized at its boiling point. Predict the signs of:

ΔSsurr

Explain your answers.

CONCEPT CHECK!

Section 17.4 Free Energy A liquid is vaporized at its boiling point. Predict the signs of:

ΔSsurr

Explain your answers.

CONCEPT CHECK!

As a liquid goes to vapor, it does work on

the surroundings (expansion occurs). Heat

is required for this process. Thus, w =

negative; q = H = positive. S = positive

(a gas is more disordered than a liquid), and

Ssurr = negative (heat comes from the

surroundings to the system); G = 0

because the system is at its boiling point

and therefore at equilibrium.

The value of ΔHvaporization of substance X is 45.7 kJ/mol,

and its normal boiling point is 72.5°C.

Calculate ΔS, ΔSsurr, and ΔG for the vaporization of one mole of this substance at 72.5°C and 1 atm.

ΔS = 132 J/K·mol

ΔSsurr = -132 J/K·mol

ΔG = 0 kJ/mol

EXERCISE!

Spontaneous Reactions

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Effect of ΔH and ΔS on Spontaneity

Section 17.5 Entropy Changes in Chemical Reactions

Gas A2 reacts with gas B2 to form gas AB at constant temperature and pressure. The bond energy of AB is much greater than that of either reactant.

Predict the signs of:

ΔH ΔSsurr ΔS ΔSuniv

Explain.

– + 0 +

CONCEPT CHECK!

Third Law of Thermodynamics

The entropy of a perfect crystal at 0 K is zero.

The entropy of a substance increases with temperature.

Standard Entropy Values (S°)

Represent the increase in entropy that occurs when a substance is heated from 0 K to 298 K at 1 atm pressure.

ΔS°reaction = ΣnpS°products – ΣnrS°reactants

Calculate ΔS° for the following reaction:

2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)

Given the following information:

S° (J/K·mol)

Na(s) 51

H2O(l) 70

NaOH(aq) 50

H2(g) 131

EXERCISE!

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Section 17.6 Free Energy and Chemical Reactions

Standard Free Energy Change (ΔG°)

The change in free energy that will occur if the reactants in their standard states are converted to the products in their standard states.

ΔG° = ΔH° – TΔS°

ΔG°reaction = ΣnpG°products – ΣnrG°reactants

A stable diatomic molecule spontaneously forms from its atoms.

Predict the signs of:

ΔH° ΔS° ΔG°

Explain.

– – –

CONCEPT CHECK!

Consider the following system at equilibrium at 25°C.

PCl3(g) + Cl2(g) PCl5(g)

ΔG° = −92.50 kJ

What will happen to the ratio of partial pressure of PCl5 to partial pressure of PCl3 if the temperature is raised? Explain.

The ratio will decrease.

CONCEPT CHECK!

Section 17.7 The Dependence of Free Energy on Pressure

Free Energy and Pressure

G = G° + RT ln(P)

ΔG = ΔG° + RT ln(Q)

Sketch graphs of:

1. G vs. P

2. H vs. P

3. ln(K) vs. 1/T (for both endothermic and exothermic cases)

CONCEPT CHECK!

The Meaning of ΔG for a Chemical Reaction

A system can achieve the lowest possible free energy by going to equilibrium, not by going to completion.

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Section 17.8 Free Energy and Equilibrium

The equilibrium point occurs at the lowest value of free energy available to the reaction system.

ΔG = 0 = ΔG° + RT ln(K)

ΔG° = –RT ln(K)

Change in Free Energy to Reach Equilibrium

Section 17.9 Free Energy and Work

Maximum possible useful work obtainable from a process at constant temperature and pressure is equal to the change in free energy.

wmax = ΔG

Achieving the maximum work available from a spontaneous process can occur only via a hypothetical pathway. Any real pathway wastes energy.

All real processes are irreversible.

First law: You can’t win, you can only break even.

Second law: You can’t break even.

As we use energy, we degrade its usefulness.

chapter 17 · pdf filechapter 17 spontaneity ... section 17.1 spontaneous processes and...

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